_oxalate.svg) | |
| Names | |
|---|---|
| Other names
Tris(oxalato)disamarium, Samarium oxalate, | |
| Identifiers | |
3D model (JSmol) |
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| ChemSpider | |
| EC Number |
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PubChem CID |
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CompTox Dashboard (EPA) |
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| |
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| Properties | |
| C6O12Sm2 | |
| Molar mass | 564.77 g·mol−1 |
| Appearance | Yellow crystals |
| Insoluble | |
| Hazards | |
| GHS labelling: | |
 | |
| Warning | |
| H302, H312 | |
| P264, P270, P280, P301+P312, P302+P352, P312, P322, P330, P363, P501 | |
| Related compounds | |
Other cations |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Samarium(III) oxalate is an inorganic compound, a salt of samarium and oxalic acid with the formula Sm2(C2O4)3.[1] The compound does not dissolve in water, forms a crystalline hydrate with yellow crystals.[2]
Synthesis
Precipitation of soluble samarium salts with oxalic acid:[3]
-
2
S
m
C
l
3
+
3
H
2
C
2
O
4
→
S
m
2
(
C
2
O
4
)
3
↓
+
6
H
C
l
{\displaystyle {\mathsf {2SmCl_{3}+3H_{2}C_{2}O_{4}\ {\xrightarrow {}}\ Sm_{2}(C_{2}O_{4})_{3}\downarrow +6HCl}}}
-
2
S
m
C
l
3
+
3
H
2
C
2
O
4
→
S
m
2
(
C
2
O
4
)
3
↓
+
6
H
C
l
{\displaystyle {\mathsf {2SmCl_{3}+3H_{2}C_{2}O_{4}\ {\xrightarrow {}}\ Sm_{2}(C_{2}O_{4})_{3}\downarrow +6HCl}}}
Also a reaction of samarium nitrate and oxalic acid in an aqueous solution:
-
2
S
m
(
N
O
3
)
3
+
3
H
2
C
2
O
4
→
S
m
2
(
C
2
O
4
)
3
↓
+
6
H
N
O
3
{\displaystyle {\mathsf {2Sm(NO_{3})_{3}+3H_{2}C_{2}O_{4}\ \xrightarrow {} \ Sm_{2}(C_{2}O_{4})_{3}\downarrow +6HNO_{3}}}}
-
2
S
m
(
N
O
3
)
3
+
3
H
2
C
2
O
4
→
S
m
2
(
C
2
O
4
)
3
↓
+
6
H
N
O
3
{\displaystyle {\mathsf {2Sm(NO_{3})_{3}+3H_{2}C_{2}O_{4}\ \xrightarrow {} \ Sm_{2}(C_{2}O_{4})_{3}\downarrow +6HNO_{3}}}}
Physical properties
Samarium(III) oxalate forms a crystalline hydrate of the composition Sm2(C2O4)3 • 10H2O with yellow crystals.
Chemical properties
Decomposes on heating:[4]
-
S
m
2
(
C
2
O
4
)
3
→
800
o
C
S
m
2
O
3
+
3
C
O
2
+
3
C
O
{\displaystyle {\mathsf {Sm_{2}(C_{2}O_{4})_{3}\ {\xrightarrow {800^{o}C}}\ Sm_{2}O_{3}+3CO_{2}+3CO}}}
-
S
m
2
(
C
2
O
4
)
3
→
800
o
C
S
m
2
O
3
+
3
C
O
2
+
3
C
O
{\displaystyle {\mathsf {Sm_{2}(C_{2}O_{4})_{3}\ {\xrightarrow {800^{o}C}}\ Sm_{2}O_{3}+3CO_{2}+3CO}}}
Crystalline hydrate Sm2(C2O4)3 • 10H2O decomposes stepwise.[5]
References
- Bulletin of the Research Council of Israel: Chemistry. Section A. Weizmann Science Press of Israel. 1959. p. 174. Retrieved 8 August 2021.
- "Samarium(III) oxalate hydrate ≥99.99% | Sigma-Aldrich". Sigma Aldrich. Retrieved 8 August 2021.
- Sanuki, Sumiko; Sugiyama, Akio; Tunekawa, Minoru; Kadomachi, Kiyotaka; Arai, Koichi (1994). "Precipitation Stripping of Samarium Oxalate from Organic Solution Containing Acid Type Extractant by Oxalic Acid". Journal of the Japan Institute of Metals. 58 (11): 1271–1278. doi:10.2320/jinstmet1952.58.11_1271. Retrieved 8 August 2021.
- Wendlandt, W. W. (1 March 1959). "Thermal Decomposition of Rare Earth Metal Oxalates". Analytical Chemistry. 31 (3): 408–410. Bibcode:1959AnaCh..31..408W. doi:10.1021/ac60147a024. ISSN 0003-2700. Retrieved 8 August 2021.
- Hussein, G.A.M.; Buttrey, D.J.; Desanto, P.; Abd-Elgaber, A.A.; Roshdy, Heba; Myhoub, Ali Y.Z. (3 June 2003). "Formation and characterization of samarium oxide generated from different precursors". Thermochimica Acta. 402 (1–2): 27–36. Bibcode:2003TcAc..402...27H. doi:10.1016/S0040-6031(02)00535-X. ISSN 0040-6031. Retrieved 8 August 2021.